The reaction
3C + D $\rightarrow$ products
Has rate = k[D] and has a half-life of 1.29 s.If initially [D] = 0.820,what is the concentration of D after 2.55 s?

Name: The reaction 3C + D $\rightarrow$ products Has rate = k[D] and has a half-life of 1.29 s.If initially [D] = 0.820,what is the concentration of D after 2.55 s?
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Question

The reaction 
3C + D $\rightarrow$ products
Has rate = k[D] and has a half-life of 1.29 s.If initially [D] = 0.820,what is the concentration of D after 2.55 s?

Quizplus · Accepted Answer

The rate law is first order in D, so the half-life is independent of [D]. The half-life is 1.29 s, so after 2.55 s, the concentration of D will be 0.25 * 0.820 = 0.21 M.

The Reaction 3C + D →\rightarrow→ Products Has Rate = K[D] and Has a Half-Life of =

The Reaction
3C + D $\rightarrow$ Products
Has Rate = K[D] and Has a Half-Life of =